Ionic bonds form between oppositely charged ions through electrostatic attraction. The strength of ionic bonds increases with greater charge separation, resulting in higher melting points. Ionic solids do not conduct electricity. Covalent bonds form when atoms share pairs of electrons to achieve stable electron configurations. Ionic and covalent bonding, as well as metallic bonding, are introduced.

1. Ionic Bonding
By: Collin Chance & Luis Marquez

3. Introduction to bonding
• An attraction between atoms that allows the
formation of chemical substances that contain
two or more atoms.
• Atoms form chemical bonds to become stable.

4. Ionic bonding
• Ionic bonds are formed between cation
and ion. Ionic bonds is a type of chemical
bond formed through an electrostatic
attraction between two oppositely
charged ions.
• Greater charge = Greater electrostatic
attraction; stronger bond = Higher
melting point

5. Ionic Bonding Continued
• The size of the ions also affect the
melting point! Ionic solids don’t
conduct electricity!

6. Covalent Bonds
• When atoms bond covalently they count a
share in the pair of electrons in the covalent
bond as two electrons in their counter shell.
• A single covalent bond is when two electrons
are shared between atoms. A double band is
when four electrons are shared and a triple is
when six electrons are shared.

7. Covalent Bonds Continued
• A sigma bond is the end to the end overlap of
the bonding orbitals, usually hybrid orbitals.
The sigma bond is a single bond. A pi bond is
the side to side overlap of hybridized p-
orbitals. Together they form a double bond.
• As bond length decreases, bond dissociation
energy increases.

8. Metallic Bonds
• A metallic bond is formed when atoms of
metal group together to for a crystal.
• Alloys- a homogeneous mixture or solid
solution of two or more metals, the atoms of
one repulsing or occupying interstitial
positions between atoms of others.